0.1868 moles
Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters ) 1.5 M KBr = moles KBr/0.025 Liters = 0.038 moles potassium bromide ------------------
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
0.29M = 0.29 moles in 1000 ml so 0.29 x 110/1000 = 0.0319 moles
Easy...the periodic table gives the average mole weight of each element averaged out over all it's naturally occurring, if any, isotopes, i.e., K is 39.09 Br is 79.9 Add them up and it's (to three significant figures): So KBr is 119 g/mole
0.1868 moles
Potassium bromide is KBr, the atomic mass of this compound is ca. 119.1. no.moles = mass/relitive molecular mass, so in this case that's 245/119.1 = 2.057 moles of KBr.
Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters ) 1.5 M KBr = moles KBr/0.025 Liters = 0.038 moles potassium bromide ------------------
First write a balanced chemical equation: 2K + Br2 ---> 2KBR Find the limiting reactant by using the moles of each element and determining which one gives you the smallest number of moles of potassium bromide. 2.92 mol K (2 mol KBr/2 mol K)= 2.92 mol KBr 1.78 mol Br2 (2 mol KBR/1 mol Br2)=3.56 mol KBr potassium is your limiting reactant so the max. number of moles of KBr that can be produced is 2.92 mol of KBr
The answer is 0,0509 mole.
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
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0.29M = 0.29 moles in 1000 ml so 0.29 x 110/1000 = 0.0319 moles
There would be 0.75 moles in 1 liter of solution. You have 100 mL which is in fact 0.1 liters. so you would have 0.1 of 0.75 moles. 0.1 x 0.75 = 0.075 moles.
Easy...the periodic table gives the average mole weight of each element averaged out over all it's naturally occurring, if any, isotopes, i.e., K is 39.09 Br is 79.9 Add them up and it's (to three significant figures): So KBr is 119 g/mole